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![1) Show that for ideal gas: [dH= Cp dT] and
dS= Cp dT/T-R dP
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- Show that = T/p for an ideal gas.Use the two appropriate values of R to determine a conversion between L. atm and J.2.25 moles of an ideal gas with Cv, m = 5R/2 are trans-formed from an initial state T= 680. K and P= 1.15 bar to afinal state I'= 298 K and P= 4.75 bar. Calculate for this pro-cess: AH & AS.
- Cp− ̄Cv=T ̄V β^2/κ reduces to ̄CP− ̄CV=R for an ideal gas.. A 2.50 mole sample of a perfect gas for which Cv,m = 3R/2 (assume constant over T-range) undergoes the following two-step process: (1) from an initial state of the gas described by T = 13 ºC and P = 1.75 x 105 Pa, the gas undergoes an isothermal expansion against a constant pressure of 3.75 x 104 Pa until the volume has doubled. (2) subsequently, the gas is cooled at constant volume. The temperature falls to -24ºC. Calculate q, w, ∆U, and ∆H for each step and for the overall process.An insulated piston is compressed to 2 atms of pressure; it has 1 mol of a gas (Cv,m = 12.5 J/K/mol) and is at room temperature (25 °C). If you suddenly let go in a room at 1 atm of pressure, what are the final values of P, T, V, ΔU, ΔH, Δq, Δw, total ΔS, surroundings ΔS, and the system ΔS? Hint: remember that ΔU = Cv×(Tf - Ti) = -Pext x (Vf - Vi); what you don’t know is the finaltemperature and volume. You have to calculate these; note that the final volume is (nRTf) / (101.325 kPa)
- Calculate the minimum constant Pext required for an isothermal compression of 1.5 mol of a vander Waals gas from 5.00 L to 0.850 L. Then, calculate w, q, and ΔU for the compression. a= 0.245 atm mol-2 L2, b=0.005 L mol-1. T=300KThe molar constant-volume heat capacity of 79.9 g Ar gas wasfound to vary with temperature according to the expression CV,m / (J K-1 mol-1) = 15.7 + 0.8 T. Calculate q,w and ∆U when the temperature is raised from 25 °C tot 110 °CShow that for an ideal gas Cp- Cv = R
- ammonia (considered to be an ideal gas) initially at 25 C and 1 bar pressure is heated at constant pressure until the volume tripled. Calculate the q per mole, w per mole, delta H, delta U, and delta S, given that CP=25.895 + 32.999 x 10-3 T – 30.46 x 10-7 (T)2 ? (J/K mol)1 kg of Air was heated at constant temperature from 0.03 m3 and 101 kPa to 0.01 m3. By how much did the internal energy change? Assume (cv = 0.7177 kJ/kg.K)12) Between 0 °C and 100 °C, the heat capacity of Hg(l) is given by: Cp,m (Hg, l) [units: J mol-1 K-1] = 30.093 – 4.944 x 10-3T Calculate ΔH and ΔS if the temperature of 1.75 moles of Hg(l) is raised from 0.00 °C to 100.00 °C at constant P.